H2 + AgCl = HCl + Ag

H_2 hydrogen + AgCl silver chloride ⟶ HCl hydrogen chloride + Ag silver

Balance the chemical equation algebraically: H_2 + AgCl ⟶ HCl + Ag Add stoichiometric coefficients, c_i, to the reactants and products: c_1 H_2 + c_2 AgCl ⟶ c_3 HCl + c_4 Ag Set the number of atoms in the reactants equal to the number of atoms in the products for H, Ag and Cl: H: | 2 c_1 = c_3 Ag: | c_2 = c_4 Cl: | c_2 = c_3 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 2 c_3 = 2 c_4 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | H_2 + 2 AgCl ⟶ 2 HCl + 2 Ag

+ ⟶ +

hydrogen + silver chloride ⟶ hydrogen chloride + silver

| hydrogen | silver chloride | hydrogen chloride | silver molecular enthalpy | 0 kJ/mol | -127 kJ/mol | -92.3 kJ/mol | 0 kJ/mol total enthalpy | 0 kJ/mol | -254 kJ/mol | -184.6 kJ/mol | 0 kJ/mol | H_initial = -254 kJ/mol | | H_final = -184.6 kJ/mol | ΔH_rxn^0 | -184.6 kJ/mol - -254 kJ/mol = 69.4 kJ/mol (endothermic) | | |

| hydrogen | silver chloride | hydrogen chloride | silver molecular entropy | 115 J/(mol K) | 96.3 J/(mol K) | 187 J/(mol K) | 42.6 J/(mol K) total entropy | 115 J/(mol K) | 192.6 J/(mol K) | 374 J/(mol K) | 85.2 J/(mol K) | S_initial = 307.6 J/(mol K) | | S_final = 459.2 J/(mol K) | ΔS_rxn^0 | 459.2 J/(mol K) - 307.6 J/(mol K) = 151.6 J/(mol K) (endoentropic) | | |

Construct the equilibrium constant, K, expression for: H_2 + AgCl ⟶ HCl + Ag Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: H_2 + 2 AgCl ⟶ 2 HCl + 2 Ag Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i H_2 | 1 | -1 AgCl | 2 | -2 HCl | 2 | 2 Ag | 2 | 2 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression H_2 | 1 | -1 | ([H2])^(-1) AgCl | 2 | -2 | ([AgCl])^(-2) HCl | 2 | 2 | ([HCl])^2 Ag | 2 | 2 | ([Ag])^2 The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([H2])^(-1) ([AgCl])^(-2) ([HCl])^2 ([Ag])^2 = (([HCl])^2 ([Ag])^2)/([H2] ([AgCl])^2)

Construct the rate of reaction expression for: H_2 + AgCl ⟶ HCl + Ag Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: H_2 + 2 AgCl ⟶ 2 HCl + 2 Ag Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i H_2 | 1 | -1 AgCl | 2 | -2 HCl | 2 | 2 Ag | 2 | 2 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term H_2 | 1 | -1 | -(Δ[H2])/(Δt) AgCl | 2 | -2 | -1/2 (Δ[AgCl])/(Δt) HCl | 2 | 2 | 1/2 (Δ[HCl])/(Δt) Ag | 2 | 2 | 1/2 (Δ[Ag])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -(Δ[H2])/(Δt) = -1/2 (Δ[AgCl])/(Δt) = 1/2 (Δ[HCl])/(Δt) = 1/2 (Δ[Ag])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| hydrogen | silver chloride | hydrogen chloride | silver formula | H_2 | AgCl | HCl | Ag Hill formula | H_2 | AgCl | ClH | Ag name | hydrogen | silver chloride | hydrogen chloride | silver IUPAC name | molecular hydrogen | chlorosilver | hydrogen chloride | silver

| hydrogen | silver chloride | hydrogen chloride | silver molar mass | 2.016 g/mol | 143.32 g/mol | 36.46 g/mol | 107.8682 g/mol phase | gas (at STP) | solid (at STP) | gas (at STP) | solid (at STP) melting point | -259.2 °C | 455 °C | -114.17 °C | 960 °C boiling point | -252.8 °C | 1554 °C | -85 °C | 2212 °C density | 8.99×10^-5 g/cm^3 (at 0 °C) | 5.56 g/cm^3 | 0.00149 g/cm^3 (at 25 °C) | 10.49 g/cm^3 solubility in water | | | miscible | insoluble dynamic viscosity | 8.9×10^-6 Pa s (at 25 °C) | | | odor | odorless | | |